Question

How many grams of phosphorus are in a sample of Ca3(PO4)2 that contains 74.0 g of calcium?

mass phosphorus = _______g

Answer #1

**we know that**

**moles = mass / molar mass**

**so**

**moles of Ca = 74 / 40**

**moles of Ca = 1.85**

**now**

**consider Ca3(P04)2**

**we can see that**

**1 mole of Ca3(P04)2 contains**

**1) 3 moles of Ca**

**2) 2 moles of P**

**3) 8 moles of O**

**so**

**moles of Ca = 3 x moles of Ca3(P04)2**

**so**

**1.85 = 3 x moles of Ca3(P04)2**

**moles of Ca3(P04)2 = 0.61666**

**now**

**moles of P = 2 x moles of Ca3(P04)2**

**so**

**moles of P = 2 x 0.61666**

**moles of P = 1.233333**

**now**

**mass = moles x molar mass**

**so**

**mass of P = 1.23333 x 31**

**mass of P = 38.233**

**so**

**38.233 grams of Phosphorus is present**

How many grams of Ca3(PO4)2 precipitate can form by reacting
169.1 mL of 1.9 M CaBr2 with an excess amount of Li3PO4, given the
balanced equation:
2 Li3PO4 (aq) + 3 CaBr2 (aq) --> 6 LiBr2 (aq) + Ca3(PO4)2
(s)

Elemental phosphorus is produced by the reaction, 2 Ca3(PO4)2 + 6
SiO2 + 10 C → 6 CaSiO3 + 10 CO + P4 Suppose that you have 9.0 moles
of Ca3(PO4)2, 21.0 moles of SiO2, and 49.0 moles of C. (a) Which
reactant is limiting? (b) What are the maximum amounts (in moles)
of CaSiO3, CO, and P4 that can be produced?

A sample contains Ca3(PO4)2, HgS, AgCl, NH4Cl, and NiS. Identify
the soluble ions after the addition of 6 MHCl; H2S and 0.2 MHCl;
OH− to a pH of 8; and (NH4)2HPO4 with NH3.
NH4Cl
HgS
Ca3(PO4)2
NiS
AgCl

How do i find the moles in Calcium Phosphate?
(Ca3(PO4)2)

solutions containing 400 g CaCl2 and 400 g Na3PO4 are mixed how
much Ca3(PO4)2 can be formed
Given equation
3CaCl2 (aq) + 2 Na3PO4 (aq) --> Ca3 (PO4)2 (s) + 6 NaCl
(aq)

Phosphorus occurs naturally in the form of fluorapatite, CaF2·3
Ca3(PO4)2, the dot indicating 1 part CaF2 to 3 parts Ca3(PO4)2.
This mineral is reacted with an aqueous solution of sulfuric acid
in the preparation of a fertilizer. The products are phosphoric
acid, hydrogen fluoride, and gypsum, CaSO4·2 H2O. Balance the
chemical equation describing this process. (Type your answer using
the format CO2 for CO2.) CaF2·3 Ca3(PO4)2(s) + (aq) + (l) (aq) +
HF(aq) + CaSO4·2 H2O(s)

1. Show the calculation of the mass of Ca3(PO4)2 needed to
make 200 ml of a 0.128 M solution.
2. Show the calculation of the volume of 0.987 M solution
which can be prepared using 24.6 grams of NaNO3.
3. Show the calculation of the volume of 0.238 M solution
which can be prepared using 13.4 grams of Ca3(PO4)2.

Solid calcium hudoxide reacts with phosphoric acid according to
the following equation:
3 Ca(OH)2+ 2H3PO4--- Ca3(PO4)2+ 6 H2O
what in volume of 0.0220 M phosphoric acid can be neutralized by
94.651 grams of Calcium hydroxide

Using the following equation
K3PO4(aq)+Ca(NO3)2(aq)---Ca3(PO4)2(s)+KNO3(aq)
If you start with 4.6 grams of CA(NO3)2 and a stoichiometric
quantity of K3PO4 and produce a 92% yield CA3(PO4)2, what is the
actual yield in grams

2 H3PO4(aq) + 3Ca(OH)2(aq) = Ca3(PO4)2 (s) + 6 H2O(l)
1.
a.Calculate the volume of .0500 M phosporic acid that would be
required to exactly react with 20.0 ml of 0.100 M calcium
Hydroxide
b. What mass of calcium phosphate will precipitate?

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